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Introduction

The smallest units into which a compound can be divided without changing its chemical properties are molecules. They are formed from combinations of atoms, the basic building blocks of all matter.

Because molecules consist of various combinations of the more than 100 kinds of known atoms, they exist in a very large number of structural forms. Molecules can form rings or chains. They can join in very long repeating structures known as polymers. In certain conditions, they can form a very precise crystal lattice. In general, the structural design of a molecule will favor the most energetically stable combination of bonds among the atoms.

Under some conditions, the same combination of atoms and bonds can result in energetically stable structures that are mirror images of one another. These are called isomers.

A molecule is not static but dynamic and constantly in motion. Its atoms rotate and vibrate around one another. The positions of the atoms, their relative motions, and their bond strengths can be changed by heat, magnetic fields, and other forces. Whether a substance will be solid, liquid, or gas under ordinary conditions depends upon the nature of the attractive forces between molecules and the freedom of the molecules to move in relation to other molecules.

Bonding and Molecular Polarity

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When atoms combine to form a molecule they either share or exchange electrons. True molecular compounds are formed when two or more atoms share electrons, resulting in what is called a covalent bond. These bonds are very strong and require a good deal of energy to break. Compounds formed with covalent bonds do not conduct electricity, and they are referred to as nonpolar because they are not very soluble in water.

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Polar molecules, on the other hand, are readily soluble in water. They are formed when atoms exchange an electron to form a bond called an ionic bond. These bonds are strong because the atoms have become more stable as a result of either losing or gaining an electron (called ionization). Molecules formed from ionic bonds are not true molecules because the electrons are not shared but exchanged.

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Compounds
formed by ionic bonding are made up of a random mixture of ions—atoms or groups of atoms that carry an electric charge as a result of having lost or gained electrons. They retain a charge because they are not bonded to the particular atom with which they exchanged electrons. An example is sodium chloride (NaCl), or common table salt. Sodium gives up an electron and becomes positively charged (Na+) when heated in the presence of chlorine. This electron is acquired by chlorine, leaving it with a net negative charge (Cl–). The resultant water-soluble NaCl is a collection of free ions that are capable of conducting an electrical current. (See alsochemistry.)

Molecular Weight

The relative molecular weight of a molecule is calculated from the sum of the relative atomic weights of its constituent atoms. For example, water (H2O) consists of two atoms of hydrogen (H2) and one atom of oxygen (O). The weight, in relative atomic weight units, of hydrogen is approximately 1 and that of oxygen about 16. Thus, the relative molecular weight of water is about 18.

Molecular weight can also be expressed in grams, in which case it is defined as the weight in grams of one mole of a substance. A mole is equal to 6.02 × 1023 units or particles. The number 6.02 × 1023 is called Avogadro’s number (seechemical element). The term 1023 means 1 followed by 23 zeros, or a billion billion times 100,000. One mole of water, or 6.02 × 1023 water molecules, weighs 18 grams.

Research

Recent research has concentrated on molecules in living organisms and the molecular reactions that govern the growth of living systems. For example, researchers study the function of the central molecule of the living cell, ATP, or adenosine triphosphate—a sort of molecular battery. A high-energy covalent bond in ATP is formed or broken to pass energy to other molecules.

Researchers also examine the nature of enzymes, the molecules within cells that alter the structure of other molecules. They are catalysts that can selectively initiate the breaking and re-forming of covalent bonds without being altered themselves.

Currently, much attention is being focused on the macromolecules that control geneticinheritance, such as deoxyribonucleic acid, or DNA, and its “messenger,” ribonucleic acid, or RNA. DNA and RNA are polymers, chains of four basic molecules, known as nucleotides, which are linked together by covalent bonds. Genetic engineers can selectively break and re-form these bonds, altering the genetic code at will.

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